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The story of sodium hexafluorophosphate goes back to the mid-twentieth century, a time when the push to explore advanced inorganic salts picked up real steam. Scientists searching for new materials to support batteries and chemical synthesis noticed a sweet spot with hexafluorophosphate compounds. In the years following World War II, research into phosphorus chemistry quickly branched out from more familiar phosphates into the world of hexafluorophosphates. Once researchers realized the relative stability and high solubility of sodium hexafluorophosphate in polar solvents, it became a candidate for energy storage and specialty chemical applications. Growth in lithium-ion battery technology shined a spotlight on hexafluorophosphates, especially as alternative or supporting electrolytes, even though sodium’s path nabbed less attention than lithium’s. Over time, advances in purification and preparation kept chipping away at obstacles. From the 1960s to now, the development around this compound highlights the steady march of material science fueled by energy demand and ambition to push chemical knowledge further.
Sodium hexafluorophosphate isn’t a household name, but it stands out in the world of salt chemistry. With the chemical formula NaPF6, its molecular structure houses a cluster of six fluorine atoms encircling a phosphorus atom, all paired with a sodium cation. This construction gives it a remarkable resistance to moisture and thermal changes when compared to many other inorganic salts. In actual practice, this compound tends to show up as a white, crystalline powder that doesn’t absorb water easily, which is a handy feature during transport and storage. As someone who has watched the commodity market for battery components, I notice how those small details – hygroscopicity, solubility, and crystal integrity – can make or break supply chain viability. These traits also open the door for its use beyond just chemistry labs and pilot facilities.
Sodium hexafluorophosphate brings a unique set of physical and chemical properties. Stable at room temperature, it withstands moderate heat without breaking down. In terms of solubility, it dissolves readily in water and many organic solvents, which allows it to act as a flexible reagent or electrolyte. This salt resists hydrolysis due to the strong P–F bonds that hold the anion together. Owing to its ionic nature, the substance acts as a decent conductor in solution, lending itself to electrochemical devices. The decomposition temperature stays above 150°C in dry air, and that thermal margin lets engineers experiment with it under conditions that might knock out more fragile options. From a visual standpoint, it stays unchanged—chalky, odorless, unreactive to the touch, with crystals that feel dense. All this makes sodium hexafluorophosphate a serious player in environments where chemical stability is prized, and I notice industrial folks like the predictability it brings.
Clarity and transparency rely on accurate labeling, a requirement in both commercial and research settings. Sodium hexafluorophosphate gets classified according to purity grades and moisture content, as contamination with other hexafluorophosphate salts or related phosphorous species can hamper performance. Typical technical specification sheets highlight minimum purity levels – pushing beyond 98% for most high-grade applications – as well as maximum traces of moisture, acids, and insoluble matter. Some industries mark the material based on its grain size and solubility in solvents like acetonitrile or dimethyl carbonate, since these details affect blending in battery electrolytes or catalysis protocols. Packaging labeling usually spells out hazard symbols too, since regulatory bodies demand vigilance when dealing with fluorinated agents. Consistent labeling standards, driven by compliance with ISO, REACH, or local chemical policies, have become a bedrock of international trade for this salt.
Preparation starts with a reaction between phosphorus pentachloride, hydrogen fluoride, and sodium chloride, where operators cautiously control conditions to encourage hexafluorophosphate formation and to fend off side reactions. Some methods swap out sodium chloride for other sodium donors, or tweak the order of reactant addition for process safety. The result brings a slurry where sodium hexafluorophosphate builds up in solution. Technicians often filter and dry the product under inert gas to prevent hydrolysis by atmospheric moisture. Every step gets recorded, as yield and purity can swing based on slight variations. Scaling up from bench to plant level highlights challenges that make preparation an art as much as a science. It’s not just chemistry; it’s about managing corrosive reagents, capturing byproducts, and straight-up patience in purification. Laboratories pursuing finer material for research prefer vacuum drying and multiple solvent washes to push for the cleanest product, while bulk manufacturers balance these steps with throughput and cost. The choice of upstream reagents affects both process risk and downstream waste, a reality manufacturers can’t ignore.
In the lab, sodium hexafluorophosphate often serves as a source of the PF6– anion. This lets researchers exchange anions in salt metathesis reactions, swap out counterions in organometallic complexes, and balance charges in mixed ionic solutions. Its reactivity springs from the stability of the PF6– group, which resists nucleophilic attack except under the most aggressive conditions. With strong bases or in hot, acidic environments, some fluoride can break free, but most reactions involving this compound look surprisingly uneventful. Chemists exploit that indifference as a feature, deploying sodium hexafluorophosphate in settings where weaker anions might decompose or throw surprises into the mix. The compound’s chemical resilience makes it an anchor in the quest for alternative ion carriers, especially as battery systems seek ways to move current without sacrificing longevity or performance. Beyond batteries, it’s a tool for shifting equilibrium in synthetic steps and for introducing fluorine, albeit through more roundabout routes than with other fluorinating agents.
Across scientific literature and industry, sodium hexafluorophosphate sometimes appears under other names. Chemically speaking, its IUPAC name spells things out as sodium hexafluorophosphate exactly, though some texts will call it sodium hexafluoridophosphate or simply NaPF6. In battery and materials circles, you can run across abbreviations like SHFP or references to simply “PF6 salts,” especially in catalogs that group this compound with lithium and potassium versions. Commercial supply lists might bundle it under various lot numbers, but the key identifiers tie back to the sodium and hexafluorophosphate content. It rarely hides behind generic branding, as most labs and engineering catalogs want clear, direct labeling to steer research or production staff away from missteps.
Fluorinated compounds demand respect, and sodium hexafluorophosphate stands out in this regard. Handling it safely isn’t something that comes as an afterthought. Direct exposure to moisture can set off toxic fumes containing hydrogen fluoride—a compound that’s infamous among chemists for its ability to burn tissue and etch glass. Even in the solid state, the salt calls for face shields, gloves, and careful air control in fume hoods. Storage involves moisture-tight containers, often under dry nitrogen or argon, especially in humid climates. In industry, safety protocols lay out not just basic chemical handling but emergency plans for accidental spillage, inhalation, or fires. The regulatory climate keeps evolving as more toxicity data emerges, but across countries, sodium hexafluorophosphate gets flagged for occupational hazard, not consumer use. Training for staff stays non-negotiable, since lapses can lead to crises. Here, I've watched safety audits clamp down on shortcuts around cleaning, labeling, and waste disposal, often driven by lessons learned the hard way.
Sodium hexafluorophosphate leaves its mark in a few key zones. In batteries, it supports the electrolyte chemistry in sodium-ion cells, a technology gaining attention as a more abundant and lower-cost alternative to lithium. Electrolytes built around NaPF6 show promising conductivity and shelf stability, fueling prototypes and bringing bench research closer to commercial viability. In the broader chemical industry, its stable anion supports a range of syntheses, especially in organometallic and coordination chemistry where the PF6– anion acts as a non-coordinating counterion. The compound crops up in catalysis, plating baths, and specialized extraction work, taking advantage of its chemical inertness in fields where unwanted reactions cost more than the reagent itself. With an eye on the future, some advanced material makers test it for use in supercapacitors and flow batteries. Adoption climbs in step with new research, and each win in pilot-stage projects builds confidence for larger infrastructure bets.
The pace of research into sodium hexafluorophosphate matches the dynamism you see across the battery materials field. Universities and corporate R&D outfits hunt for ways to push its conductivity, fine-tune solubility in next-gen solvents, and pare down synthesis costs. Teams experiment with blending it into new electrolyte cocktails that use additives to suppress dendrite formation or widen the operational temperature bandwidth for sodium-ion batteries. Some labs dig into the compound’s ability to serve as a supporting salt in nonaqueous redox flow systems. Others revisit the nuts and bolts of production, looking for greener synthesis paths that cut down on energy use or hazardous byproducts. The desire to scale up sodium-ion technology for grid storage keeps this area lively, especially as market forces and policy watchers look for battery solutions that dodge lithium supply constraints. Publications roll out new data on electrochemical stability, corrosion impact, and even crystal engineering—knowledge that, frankly, feels overdue in the public domain. Each advance in the lab sparks questions about scale-up, real-world cycling stability, and compatibility with evolving anode and cathode designs. Progress tails the larger uptick in sodium-based technologies, but the energy and curiosity in the field jump out at technical conferences and patent filings.
Toxicity research on sodium hexafluorophosphate lags behind its more common cousins like sodium fluoride, but there’s enough knowledge to guide caution. The biggest red flag centers on its ability to release hydrogen fluoride on decomposition, especially in reaction with water or under strong heat. HF gas can do severe damage to lungs, eyes, and skin, so most risk assessments treat exposure with the same care as other high-hazard materials. Ingestion can lead to acute poisoning, mainly if breakdown products are present, while chronic workplace exposure might edge risk higher due to cumulative fluoride intake. Ecological impact shows up in poor aquatic biodegradability and potential bioaccumulation challenges for wildlife if spills occur. Waste handling procedures call for neutralization and secure containment, guided by studies of aquatic and soil persistence. Field studies keep adding nuance, but the precautionary approach dominates company policy right now. Experience shows overconfidence in lab settings breeds more incidents than overly strict safety protocols, a balancing act that shapes research culture wherever sodium hexafluorophosphate appears.
Eyes turn toward the future as sodium hexafluorophosphate rides a wave of curiosity linked to sodium-ion batteries and resource diversification in energy storage. A lot of investors and scientists ask if this compound can help fill the gap left by high lithium and cobalt prices, especially for large-scale power grids and backup systems. Advances in green synthesis, dust reduction, and lower-moisture processing promise to make handling safer and manufacturing more sustainable. Regulatory clarity keeps pushing producers toward safer, lower-impact pathways, which, in turn, may open the door for scaling up beyond the handful of specialty producers active today. While established applications in research and industry remain steady, the pressure comes from both sides—market buyers need reliability, and environmental groups demand stewardship. New electrolyte formulations, broad testing in pilot batteries, and better toxicity data will drive decisions during the next decade. Staying ahead means keeping up with research, treating worker health as a long-term investment, and resisting the urge to cut corners in quality or transparency.
Grab a modern device—anything from a high-performance electric car to the smartphone buzzing on your desk—there’s a good chance the battery inside it contains sodium hexafluorophosphate (NaPF6). For years, lithium-ion batteries have fueled a tech revolution. People rarely peek behind the screen, but inside, the electrolyte needs a stable, ion-conducting salt. Sodium hexafluorophosphate does this job well. It offers solid chemical stability, even at the high voltages demanded by today’s electronics. Without a salt like this, charge cycles degrade fast, leading to sluggish performance and shorter device lifespans.
I remember troubleshooting an EV battery lab project where early prototypes would lose significant charge after just a couple of months. Switching to NaPF6 cut down on these problems, letting us focus less on breakdowns and more on improving range. Companies like Panasonic and LG Chem rely heavily on this compound in their battery supply chains.
Students and researchers mix this compound in labs nearly every day. In chemistry departments, NaPF6 gives budding scientists a reliable way to test reaction mechanisms or run experiments where they need a non-interfering, non-coordinating anion. Saying this from experience, the way NaPF6 dissolves in different solvents can teach a lot about ion conductivity and solvent compatibility. Not every salt gives these reproducible results.
Academic research into next-generation batteries, solar energy storage, and even supercapacitors often starts with sodium hexafluorophosphate. Early results appear in the literature, shaping commercial battery designs years down the road.
Europe and Asia have both ramped up their electric mobility goals in the last decade. You see growing demand in Germany, South Korea, and China. Their battery factories call for tons of NaPF6 every year. I saw it firsthand while touring facilities near Suzhou, where the sheer volume of precursor chemicals flowing through the plant feels staggering. Huge international suppliers build distribution centers just to keep up with battery gigafactories, preventing production slowdowns.
With all these uses, it’s fair to ask about the impact on the planet and our health. Sodium hexafluorophosphate breaks down into fluorides if mishandled and releases toxic gases at high temperatures. People working with it need gloves, goggles, and plenty of ventilation. Regulations in the EU and US outline strict safety and disposal rules to keep workers and communities safe.
Researchers keep hunting for greener alternatives, such as lithium bis(fluorosulfonyl)imide or other less hazardous salts. Adoption looks slow, though. Cost, supply chain lock-in, and years of battery field data mean NaPF6 isn’t leaving center stage overnight. Cleaner production practices and better recycling could soften the footprint, but there’s work ahead.
Sodium hexafluorophosphate sounds like something you’d stumble across in a chemistry textbook. In reality, most people come across this chemical inside lithium-ion batteries, not tucked away in kitchen cabinets. Its main job: shuttling ions back and forth so phones, laptops, and e-bikes do what they do. As handy as it is for charging up our gadgets, questions swirl about what happens if this material ends up where it shouldn’t.
During my college years, lab safety rules drilled into us weren’t just for show. Accidents always seemed to happen when someone got a little too comfortable. Handling sodium hexafluorophosphate meant lab goggles and gloves, even with tiny samples. Even if it acts stable most of the time, mixing it with water or acid changes the equation. Out comes toxic gas — hydrogen fluoride — which attacks the skin, eyes, and lungs. I remember working around fluoride compounds and learning just how much pain and injury contact could cause. No amount felt small if safety got ignored. Skin blisters, eye irritation, and lung burning could start after only a brief mistake. The real danger comes from what you can’t see or smell right away.
Production of batteries doesn’t slow down, so warehouse handlers, warehouse workers, even first responders in emergencies run into this chemical more often. In fires involving these batteries, sodium hexafluorophosphate spills risk combining with water from sprinklers or rain. Then the poisonous gas escapes, and people nearby breathe it in without warning. Even solid pieces don’t stay harmless—sweaty palms or wet floors can trigger problems. Decades ago, few people thought about these chemicals outside big factories, but that’s changed. Now, supply chains and recycling plants fill with these salts. Reports of acute fluoride exposure, skin burns, and even permanent lung damage come up in hospital records. One study in the journal “Occupational Medicine” tied accidental exposure to long-term respiratory issues for workers at battery recycling sites.
Manufacturers claim regular use doesn’t threaten customers since the material stays locked inside batteries—nothing leaks out during charging or use. That much rings true if devices stay intact. The nightmare plays out when batteries break open due to dropping, crushing, or overheating in fires. Recyclers and repair shop workers take the brunt of it, breathing dust or vapors nobody notices at first. Chronic exposure even at lower levels sets off concerns about teeth, bone, and thyroid health over time. Most cases don’t make the news, but folks dealing with battery waste, from warehouse staff to repair techs, have raised questions at every safety briefing I’ve attended.
Mitigating risk means more than shipping pamphlets with safety data. In places I’ve worked, switching gloves from latex to thicker nitrile helped cut contact. Real-time air quality monitors caught leaks we never noticed before. Training workers on spill response made accidents less likely to turn ugly. Companies owning battery collection points have started installing better ventilation and keeping calcium gluconate gel handy—a life-saver for exposed skin. Regulators lean on labeling rules and emergency reporting, but businesses shouldn’t wait for fines to ramp up education or invest in safety gear. Personal experiences dealing with nervous colleagues underline the need for transparency, regular safety drills, and honest reporting of mishaps. Batteries power progress, but the chemicals inside deserve respect and careful handling to avoid harm as demand grows.
Anyone who works with lithium-ion batteries, specialty glass, or industrial electrolytes knows about sodium hexafluorophosphate. Its usefulness in research and industry comes with a heavy dose of caution. I’ve seen what happens when someone treats it like any other lab powder—cloudy air, irritated eyes, and a hasty evacuation. A chemical like this calls for respect, not just a spot on the shelf.
Sodium hexafluorophosphate releases hazardous gases, including hydrogen fluoride, when it meets water or even just humid air. I remember once spotting a bag left ajar on a muggy afternoon; the smell gave it away right away, and the corrosion on nearby metal left a permanent reminder of what can go wrong. Aside from ruining equipment, improper storage can trigger health problems—burns, lung trouble, and lasting chemical exposure. That’s not a risk anyone should run.
Dry, cool, and airtight—those are the non-negotiables. For starters, glass bottles with sturdy seals work best. Plastic, especially polyethylene containers, holds up too. Metal containers would set off a chain reaction, so those stay out of the picture. Desiccators with fresh drying agents go a long way in stopping moisture before it gets near the powder. I always double up on sealing bags and tuck the bottle into a desiccator, just to cut down on the odds of a leak or accidental exposure.
Good storage also means keeping the chemical away from anything acidic or anything that might catch fire. I keep my sodium hexafluorophosphate on a dedicated shelf, far from solvents and strong acids. This helps stop nasty gas releases from sneaky cross-reactions. Mark the container clearly, so nobody stumbles onto it unaware. The few seconds it takes to label something can prevent a world of trouble down the line.
If you’ve ever had to respond to a chemical spill, you know it’s not just about keeping the lab safe. We owe it to ourselves to protect the wider environment. Sodium hexafluorophosphate poses a serious risk if it makes its way into drains or groundwater. Never store it where a drop could roll down a sink or reach soil. Labs I’ve worked in always use secondary containment—trays, bins, or dedicated cabinets—to catch any container leaks.
Regular checks pay off. At least once a month, I inspect seals and drying agents. A little patch of haze inside a bottle or a cloud under the cap calls for immediate action. Bad storage can sneak up quietly, but the cost comes loud and clear: damaged gear, burned skin, and piles of paperwork. Using gloves, goggles, and a good fume hood shouldn’t just be a rule; it belongs in every single handling routine.
Training makes all the difference. I've seen accidents traced back to a researcher who never learned the right handling steps. Hands-on instruction and regular safety briefings help everyone spot trouble before trouble spots them. Switching to smaller containers for daily use also limits the fallout if a spill does happen. Large stock can stay locked away while a small working sample covers the day’s needs.
Storing chemicals like sodium hexafluorophosphate isn’t about ticking boxes for compliance. It’s about protecting people, equipment, and the spaces where good work happens. Taking those extra steps never feels like wasted effort. In my experience, diligence equals safety, every time.
Sodium hexafluorophosphate shows up in labs as NaPF6. Each unit carries a single sodium atom (Na), a phosphorus atom (P), and six fluorine atoms (F). Naming in chemistry often confuses people, but here it’s pretty clear: sodium as the cation pairs with the hexafluorophosphate anion (PF6-). This salt tends to appear as a white, crystalline solid and dissolves well in water and polar organic solvents.
Chemistry class might seem dry, yet this salt keeps cropping up across industries. Labs use it a lot to study ionic conductivity. The battery world finds it especially useful as a supporting salt in lithium-ion cells. Lithium batteries take off thanks in part to electrolytes like sodium hexafluorophosphate. The salt’s stable, tough, and keeps ions flowing between a battery’s terminals. In real-world terms, it helps keep your phone on longer and your car moving farther if you drive electric.
Engineers favor sodium hexafluorophosphate because it boosts energy densities and battery lifespan. As mobile devices and electric vehicles push for longer runtimes, the demand for more efficient battery electrolytes climbs. NaPF6 isn’t perfect—moisture and high voltages can break it down—but researchers keep refining how it’s used. Safe handling in the factory means storage in dry places to keep degradation at bay. A faulty electrolyte won’t just lower performance; it can lead to short circuits and fires. For anyone in science or engineering, missteps in this space could mean higher risks and wasted resources.
Sodium hexafluorophosphate doesn’t belong near bare hands or in open air for long. Fluorine’s chemical power means it reacts fast, especially if moisture sneaks in. PF6- breaks up and releases hydrogen fluoride (HF) gas, which stings the nose and eyes and eats away at many materials. Chemical burns and inhalation risks make careful lab habits vital. Labs need protocols: gloves, good ventilation, and sealed storage keep accidents rare.
Concerns reach past personal safety. Fluorinated compounds stick around in the environment. Once sodium hexafluorophosphate escapes, it can pollute water and soil. Waste treatment systems struggle with persistent fluorine byproducts. Some scientists push for greener alternatives, looking at less-reactive salts or recyclable electrolyte systems. The transition takes time, but industry and regulators have both started testing new, sustainable solutions to cut down on hazardous waste.
Finding replacements for sodium hexafluorophosphate will need research and investment, not just industry tweaks. Collaboration between chemical engineers, battery manufacturers, and environmental health specialists creates new paths forward. My own experience saw projects stall when teams overlooked the disposal process—a clear case for fully integrating safety into early design stages.
For now, those handling NaPF6 can focus on airtight storage, rigorous workplace training, and proper disposal channels. Regular audits and hazard reviews shine light on overlooked leaks or misused chemicals. And as everyday devices push for higher power, the pressure mounts to put safety and sustainability up front rather than trying to fix problems after the fact.
Working with sodium hexafluorophosphate, people face hazards that aren’t always clear until something goes wrong. Coming from years of mixing, storing, and sometimes cleaning up after chemicals just like this, I’ve seen how skipping over the right gear or ignoring protocols leads to trouble that usually stays with you longer than any job assignment.
The safety data sheet for sodium hexafluorophosphate picks out the main dangers right from the start: eyes, skin, lungs. Contact brings burning, itching, and if you’re unlucky enough to breathe the dust for a whole shift, coughing turns into real lung pain. Some folks still think wearing goggles and gloves slows them down, but after a few close calls, nobody in my crew skips any of that anymore. Nitrile gloves, chemical splash goggles, and a lab coat hang by the entry for a reason — you only need to get a little of this stuff on you once for your whole routine to change.
Skin and eyes can’t shrug off sodium hexafluorophosphate. Any splash stings bad, and sometimes folks rush to the eye wash, hoping they react fast enough. Water works for flushing, but only if you do it for a solid fifteen minutes or more. On skin, the sensation doesn’t fade fast, and irritation lasts well into the next day. Repeated exposure roughens hands, so it pays to check gloves for holes. No shortcut pays off if you’re itching for hours or worse, making a visit to urgent care.
People come to work thinking a dust mask counts as protection, though the SDS calls for a NIOSH-approved respirator when dust could fly. Airborne sodium hexafluorophosphate tastes metallic, and coughing sets in quicker than most expect. Poor ventilation means you’re asking for a sore throat or worse, long-term lung trouble. After a couple weeks in a lab with underpowered fans, coughing turned into bronchial irritation that took me out for days. Keeping extraction vents clear and running makes the air safe for everyone, not just the person handling the powder.
Storing sodium hexafluorophosphate in a tightly sealed, clearly labelled container keeps trouble away from the start. Any contact with moisture means hydrofluoric acid might form, which is even riskier. Spilled powder gets swept up with a dustpan, never a vacuum, and put in a plastic drum with a secure lid. Trying to clean up using anything wet turns a spill into something much worse. My shop runs on clear labeling, up-to-date spill kits, and no nonsense about skipping spill responses. Every few months, we review these steps, because old habits die hard and new hires don’t always see the fuss until an accident hits home.
Disposing of sodium hexafluorophosphate isn’t like tossing out regular trash. Qualified hazardous waste service takes priority. Trying to rinse it down a drain or mixing it with landfill trash risks more than fines — it puts the next crew, city workers, or kids at risk. Experience in waste management reminded me how little mistakes with disposal linger in water systems or soil for generations.
Even if people only handle sodium hexafluorophosphate for a quick batch or lab project, each line of that SDS stands for a pain point that could have been avoided. The solution starts with real training, better gear, and respect for the rules. Everybody deserves to go home with no unexpected burns, coughs, or long-term health bills. Over time, it’s the basics — gear up, label clearly, and keep the air moving — that keep hands safe, lungs clear, and careers unbroken.
| Names | |
| Preferred IUPAC name | Sodium hexafluorophosphate |
| Other names |
Phosphoric acid hexafluorine sodium salt Sodium phosphate hexafluoride |
| Pronunciation | /ˌsoʊdiəm ˌhɛksəflʊəˈrɒsfət/ |
| Identifiers | |
| CAS Number | ['16893-85-9'] |
| Beilstein Reference | 683122 |
| ChEBI | CHEBI:76041 |
| ChEMBL | CHEMBL1201571 |
| ChemSpider | 82518 |
| DrugBank | DB11266 |
| ECHA InfoCard | '03c20baa-d6b3-4e36-9c81-6369a977cfba' |
| EC Number | 232-608-7 |
| Gmelin Reference | 85350 |
| KEGG | C14597 |
| MeSH | D017766 |
| PubChem CID | 24854 |
| RTECS number | SC9100000 |
| UNII | Q69E8R8994 |
| UN number | UN1457 |
| Properties | |
| Chemical formula | NaPF6 |
| Molar mass | 167.95 g/mol |
| Appearance | White crystalline powder |
| Odor | Odorless |
| Density | 1.522 g/cm³ |
| Solubility in water | Soluble in water |
| log P | -4.0 |
| Acidity (pKa) | ~7 |
| Basicity (pKb) | 11.71 |
| Magnetic susceptibility (χ) | -62.0·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.333 |
| Viscosity | 1.74 mPa·s (at 25 °C, water solution, 10%) |
| Dipole moment | 0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 165.1 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | –1615 kJ/mol |
| Pharmacology | |
| ATC code | A01AD11 |
| Hazards | |
| Main hazards | Toxic if swallowed, causes severe skin burns and eye damage, may cause respiratory irritation |
| GHS labelling | GHS05, GHS07 |
| Pictograms | GHS05,GHS07 |
| Signal word | Warning |
| Hazard statements | H301 + H311 + H331: Toxic if swallowed, in contact with skin or if inhaled. H373: May cause damage to organs through prolonged or repeated exposure. |
| Precautionary statements | P261, P264, P271, P272, P273, P280, P301+P330+P331, P302+P352, P304+P340, P305+P351+P338, P312, P314, P321, P330, P362+P364, P403+P233, P405, P501 |
| NFPA 704 (fire diamond) | Health: 2, Flammability: 0, Instability: 1, Special: - |
| Autoignition temperature | > 500 °C |
| Lethal dose or concentration | LD50 (oral, rat): > 1700 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral-rat LD50: 50 mg/kg |
| NIOSH | TT21000 |
| PEL (Permissible) | PEL: 2.5 mg/m³ |
| REL (Recommended) | 2.5 mg/m³ |
| IDLH (Immediate danger) | 30 mg/m3 |
| Related compounds | |
| Related compounds |
Sodium fluoride Ammonium hexafluorophosphate Potassium hexafluorophosphate Lithium hexafluorophosphate |
